Objectives: i. Outline the steps in the manufacture of ammonia from its elements, by the Haber Process. ii. Discuss the uses of ammonia iii. Assess the.

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Presentation on theme: "Objectives: i. Outline the steps in the manufacture of ammonia from its elements, by the Haber Process. ii. Discuss the uses of ammonia iii. Assess the."— Presentation transcript:

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Objectives: i. Outline the steps in the manufacture of ammonia from its elements, by the Haber Process. ii. Discuss the uses of ammonia iii. Assess the impact of the ammonia industry on the environment

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Le Chetalier’s Principal:  PRESSURE-increasing the pressure causes the equilibrium position to move to the right resulting in a higher yield of ammonia since there are more gas molecules on the left hand side of the equation (4 in total) than there are on the right hand side of the equation (2). Increasing the pressure means the system adjusts to reduce the effect of the change, that is, to reduce the pressure by having fewer gas molecules.

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 TEMPERATURE-Decreasing the temperature causes the equilibrium position to move to the right. Resulting in a higher yield of ammonia since the reaction is exothermic (releases heat). The system will produce more heat since energy is a product of the reaction. and therefore will produce more ammonia gas.

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Rate Considerations:  CATALYST- ensures that the reaction is fast enough for a dynamic equilibrium to be set up within the very short time that the gases are actually in the reactor.  PRESSURE- increasing the pressure brings the molecules closer together. In this particular instance, it will increase their chances of hitting and sticking to the surface of the catalyst where they can react. The higher the pressure the better in terms of the rate of a gas reaction.

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 TEMPERATURE- a higher temperature is used to speed up the reaction which results in a lower yield of ammonia. Increasing the temperature, more reactant molecules have sufficient energy to overcome the energy barrier. A temperature range of °C is a compromise designed to achieve an acceptable yield of ammonia (10-20%) within an acceptable time period.

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SUMMARY OF THE HABER PROCESS

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Agriculture and Fertilizer Industry: Can be applied directly to the soil as liquid ammonia Can be used to produce fertilizers such as urea, ammonium and nitrate salt. As a source of protein in livestock feeds for cattles, sheep and goats.

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Chemical Industry: To manufacture nitric acid which is used to make explosives To neutralize acid constituents of crude oil and to protect equipment from corrosion As a refrigerant because it easily liquefied by compression or cooling and absorbs large amount of heat from its surroundings The manufacture of certain products such as sulfa drugs, vitamins and cosmetics Weak ammonia solutions are also widely used as commercial and household cleaners and detergent.

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Plants and Animals: Ammonium nitrate fertilizers are water soluble and easily washed out from farmlands into waterways. When this occurs over a period of time, it leads to a rapid algal growth known as EUTROPHICATION. This prevents light from reaching lower plants in the water. The plants die and bacteria uses the dissolve oxygen. Without oxygen, aquatic organisms also die.

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Humans. Humans: HIGH CONCENTRATION LOW CONCENTRATION TREATMENT InhalationImmediate burning of the nose, throat and respiratory tract. Coughing, nose and throat irritation. Dispense humidified oxygen, bronchodilators and airway management. Skin/ Eye contactSevere injury and burns permanent eye damage or blindness. Rapid skin or eye irritation Decontaminate eyes with copious amounts of water. IngestionCorrosive damage to the mouth, throat and stomach. In infants, nitrates easily combine with heamoglobin resulting in methaemoglobinaemia syndrome. Nitrates are carcinogenic- they react with amines in the diet to form carcinogenic compounds. Ingested ammonia is diluted with milk or water